Lect+27+08

# Lect+27+08 - Objectives for Kinetics Lecture 27 A plain...

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Objectives for Kinetics - Lecture 27 A plain language understanding of Rate laws Reaction orders Behavior of first order reactions Behavior of homogeneous second order reactions Reaction mechanisms Elementary Reaction processes Kinetics and chemical equilibrium

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Concentration versus time Reactants NO 2 (g)+CO(g) CO 2 (g) +NO(g) Products Rate = - d[NO 2 ]/dt = - d[CO]/dt = +d[NO]/dt= +d[CO 2 ]/dt
Rates of Reaction Remember to include the reciprocal of the stoichiometric coefficients aA + bB cC + dD Rate = -(1/a) d[A]/dt = -(1/b) d[B]/dt = +(1/c)d[C]/dt = +(1/d)d[D]/dt

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Reaction Orders For the reaction aA products Generally the rate is expressed in terms of the concentration of reactant(s) Rate = k[A] n where ‘n’ is the reaction order. Negative first order Rate = k[A] -1 Negative half order Rate = k[A] -1/2 Zero order Rate = k[A] 0 = k Half order Rate = k[A] 1/2 First order Rate = k[A] 1 Second order Rate = k[A] 2 Reaction orders must be determined experimentally
Partial and Total Reaction Orders For the reaction A products If rate = k[A], then total reaction order is 1 and the partial order with respect to A is 1 For the reaction A+B products If rate = k[A][B], then the total reaction order is 2 The partial order with respect to A is 1 and partial order with respect to B is 1. If rate = k[A]/[B], then the total reaction order is 0 The partial order with respect to A is 1 and partial order with respect to B is -1.

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• N 2 O 5 products Plot of ln[N 2 O
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